1. ATOMIC ORBITALS Schrodinger’s Quantum Mechanics Model

2. ORBITALS – AREAS WITHIN ATOMS WHERE THERE IS A HIGH PROBABILITY OF FINDING ELECTRONS  Principal Energy Levels - A region around the nucleus of an atom where the electron is likely to be moving. (n = 1, 2, 3, 4, etc.)  Number 1-7 on periodic table down side.

3. ENERGY SUBLEVELS  Energy sublevels can be thought of as a section of seats in a theater. The rows that are higher up and farther from the stage contain more seats, just as energy levels that are farther from the nucleus contain more sublevels.  Sublevels are labeled s, p, d, and f according to the shapes of the atom’s orbitals.

4. ATOMIC ORBITALS  Each orbital may contain at most 2 electrons.  Each energy level may contain at most 1 s orbital, 3 p orbitals, 5 d orbitals, and 7 f orbitals. (all odd numbers). Energy Level# of Sublevels (types of orbitals present) # of Orbitals# of Electrons 1 s12 2 spsp 1 s 3 p 8 3 spdspd 1 s 3 p 5 d 18 4 spdfspdf 1 s 3 p 5 d 7 f 32

5. LABEL AND OUTLINE THE S, P, D, AND F BLOCKS ON THE PT AS SHOWN BELOW (ANY 4 COLORS)

6. LABEL THE SUBLEVELS (1S, 2S, ……)

7. PRACTICE: READ LIKE A BOOK  Hydrogen (1 electron) : 1s 1  Helium(2 electrons): 1s 2  Lithium(3 electrons): 1s 2, 2s 1  Beryllium(4 electrons): 1s 2. 2s 2  Carbon(6 electrons): 1s 2, 2s 2, 2p 2  Iron(26 electrons): 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 6  You try: Sulfur ( ___ electrons): _____________________  Bromine (___ electrons): _______________________

8. MORE PRACTICE  Do page 9 that you got yesterday. “Practice #1 – electron configuration”